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ECAT Chemistry Chemical Equilibrium Test Online

Maan AliLast Updated: April 19, 2025

Chemistry Chemical Equilibrium MCQS Online Test

ECAT Chemistry Chemical Equilibrium Chapter Online Test

Total Questions:	63
Time Allowed:	30 Minutes
Total Marks:	63
How to Attempt Test:	Please choose the right Option in MCQ-type question.
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ECAT Chemistry Chemical Equilibrium Test

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Page 1 of 3

Chemistry

1. At start of reaction, concentration of reactants are on

Lower side

Higher side

Optimum side

Constant

2. When ever a week a base is dissolved in water, it gives its conjugate acid similarly a weal acid in water products its conjugate base. The conjugate acid base pair is stated by

Le – Chatelier’s principle

Law of mass action

Lowery Bronsted concept

Common on effect

3. Synthesis of ammonia by Habor process is an example of ___________

Irreversible Reaction

Constant Reaction

Decomposition Reaction

Reversible Reaction

4. In an exothermic reaction, a 10° rise in temperature will

Decrease the value of equilibrium constant

Double the value of Kc

Not produce any change in Kc

Produce some increase in Kc

5. By the addition of base in water pH will be

No effect

Equal to 7

More than 7

Less than 7

6. In reversible reactions, if the forward reaction occur very fast then reactant (s) is (are) __________

Unstable

Solids

Stable

At very high temperature

7. In an exothermic reversible reaction increase in temp shifts the equilibrium to

Reactant side

Fluctuate

Remains unchanged

Product side

8. Which set of solutes will form a buffer when dissolved in water to make 1 litter of solution?

0.0002M HCl

0.4 mole of CH3COOH with 0.4 mole of NaOH

0.2 mole of NaCl with 0.2 mole of HNO3

0.4 mole of NH3 with 0.2 mole of HCl

9. Which of the following is more acidic?

Apples

Bread

Bananas

Lemons

10. Preparation of buffer solution can be done by mixing

Weak base and its salt with strong acid

Strong acid and its salt with weak base

Weak acid and its salt with weak base

Strong base and its salt with weak acid

11. In which of the following cases, the reaction goes farthest to completion?

K = 10¯²

K = 10³

K = 10⁰

K = 10

12. Who studied the effect of temperature on equilibrium?

Lewis

Vant Hoff

Van der Waal

Arrhenius

13. What is the relationship between kp and kc?

Kc - kp (RT)∆n

kp = kc (RT)∆n

kp = kc (RT)-∆n

kc = kp (P)-∆n

14. Kc > Products / Reactants favours

Equilibrium

Reaction completed

Backward reaction

Forward reaction

15. Solubility of any salt can be determined from

Ksp

16. Water and ice are in equilibrium at 0C° and pressure is applied at this stage, then

Water evaporates

Equilibrium is not disturbed

More ice is formed

More water is formed

17. Reaction which proceed in both the directions is called

Reversible

Non spontaneous

Irreversible

Spontaneous

18. Two moles of HI was heated in a sealed tube at 440°C till the equilibrium was reached. HI was found to be 22% decomposed. The equilibrium constant for dissociation is

0.0796

0.282

1.99

0.0199

19. The reaction 2SO₂ + 2O₂ ⇌ 2SO will be favoured by

High temperature and low pressure

High temperature and high pressure

Low temperature and low pressure

Low temperature and high pressure

20. The equilibrium constant in a reversible chemical reaction at a given temperature

Is not characteristic of the reaction

Does not depend on the initial concentrations of reactants

Depends on the initial concentration of the reactants

Depends on the concentration of one of the products at equilibrium

21. AgCl dissolved with cone (2 x 10¯²) Ksp will be

4 x 10¯⁴

3.6 x 10¯⁵

3.6 x 10¯⁶

7.2 x 10¯⁶

22. A buffer solution can be prepared by mixing

A weak acid and weak base

A strong acid and weak base

A strong acid and its salt

A weak base and its salt with strong acid

23. The state of equilibrium refers to

Dynamic state

Stationary state

State or rest

State of inertness

24. The rate of chemical reaction is directly proportional to the active mass of reactant this statement is known as ___________

Law of reaction

Law of Equilibrium

Law of Mass Action

None of these

25. Addition of CH3COOH and CH3COONa gives in water

Standard solution

Both b and c

Buffer solution

Acidic buffer solution

Page 2 of 3

26. Temperature for preparation of SO₃ is

400 °C

200 °C

400 – 500 °C

600 °C

27. Which statements are correct for a reaction at equilibrium?
(I) The forward and reverse reactions both continue
(II) The rates of the forward and reverse reactions are equal
(III) The concentrations of reactants and products are equal

I and III only

I and II only

II and III only

I, II and III only

28. The relationship between Kp and Kc is give by

Kp = Kc (RT)∆n

Kc = Kp (RT)∆n

Kp = Kc (RT)∆

Kp = Kc (RT)-∆n

29. When pressure is applied to the equilibrium system Ice ⇌ Water? Which of the following phenomenon will happen?

More water will be formed

Water will evaporate

Equilibrium will not be formed

More ice will be formed

30. In reversible reaction the changes in forward and backward reaction occur _________

Both a and b

Simultaneously

Individually

None

31. In a chemical reaction N₂ + 3H₂ ⇌ 2NH₃ at equilibrium point

The reaction has stopped

Equal masses of N₂ and H₂ are reacting

Equal volumes of N₂ and H₂ are reacting

The same amount of ammonia is formed as is decomposed into N₂ and H₂

32. Which of the following aqeous solution will be basic?

Na₂CO₃

Na₂SO₄

Fecl₃₋

NaCl

33. Conjugate base of a very weak acid is

Do not ionize

Salt

Weak base

Strong base

34. Which pH is considered as basic?

35. Idea of PH and POH was put forward by

Sorenson

Chadwiick

Einstein

Gibbs

36. At certain temperature, 50% of HI is dissociated into H₂ and I₂ the equilibrium constant is

1.0

0.25

0.5

3.0

37. When sparingly soluble salt is in equilibrium with molar concentration of its oppositely charged ion when the product is called

Common ion effect

Dissociation constant

Dissociation constant for an acid

Solubility product

38. For the reaction 2A(g) + B(g) ⇌ 3C(g) + D(g) two moles each of A and B were taken into a flask. The following must always be true when the system attained equilibrium

[A] > [C]

[B] = [C]

[A] < [B]

[A] = [B]

39. If rate of concentration of reaction is equal to rate of concentration of products in reversible reaction the __________

Reaction goes backward

Equilibrium will established

Reaction stops after some time

Reaction goes forward

40. Which one of the following is a buffer solution?

Brine

Blood

Solution of CuSO4

Glue

41. If a buffer solution of higher PH than seven is to be made we use

Strong acid and strong base

Weak base and its salt with a strong acid

Weak acid and strong base

Weak acid and its salt with a strong base

42. The rate at which a substance reacts is directly proportional to its active mass and the rate of reaction is directly proportional to the product of the active mass of reacting substances is known as

Law of conservation of energy

None of all

Le – Chatelier’s principle

Law of mass action

43. Which of the following factors will favour the reverse reaction in a chemical equilibrium?

Removal of one of the products regularly

None of these

Increase in concentration of one of the reactants

Increase in concentration of one of the products

44. When H₂ and I₂ are mixed and equilibrium is attained, then

The reaction stops completely

HI dissociation stops

Amount of HI formed is equal to the amount of H₂ dissociated

None of these

45. An equilibrium constant of 10¯⁴ for a reaction means that the reaction is

One that will have 50% product and 50% reactant at equilibrium

One that is unfavourable and will not have very much product at equilibrium

The equilibrium constant only relates to the speed of a reaction and not to the amount of product formed

One that is very favorable and will have mostly product at equilibrium

46. When rate of forward reaction is equal to rate of backward reaction, then the equilibrium established is called

Static equilibrium

None of all

Dynamic equilibrium

Chemical equilibrium

47. Which of the following gives a basic buffer?

NH₄OH + NH₄Cl

NaOH + NaCl

NaOH + CH₃ COONa

NaCl + CH₃ COOH

48. A basic Buffer solution can be prepared by mixing

Weak acid and its slat with strong base

Strong base and its salt with weak acid

Strong acid and its slat wit weak base

Weak base and its salt with strong acid

49. When pressure is applied to the given equilibrium ice water which of the following will happen

More ice will be formed

More water will be formed

Equilibrium will not be disturbed

Water will formed

50. For equilibrium 2NO₂(g) ⇌ N₂O₄(g) + 14.6 kcal increase of temperature would

Not alter the equilibrium

Stop the reaction

Favour the decomposition of N₂O₄

Favour the formation of N₂O₄

Page 3 of 3

51. PH of human blood is

7.80

7.00

7.35

7.50

52. If the value of kc is very low then the forward reaction will occur __________

Fast

Slowly

Moderately

Randomly

53. For a reaction H₂ + I₂ ⇌ 2HI at 721 K, the value of equilibrium constant is 50. If 0.5 moles each of H₂ and I₂ is added to the system the value of equilibrium constant will be

0.2

0.02

54. What can affect the magnitude of equilibrium constant Kp of a reversible gaseous reaction

Catalyst

Temperature

None of these

Pressure

55. The equilibrium will shift towards right by increasing ___________ of reactants

Concentration

Pressure

Impurity

Temperature

56. Le-Chatelier’s principle is sometime known as

Law of mobile equilibrium

All of these

Law of mass action

Law of active mass

57. pH of milk is

7.5

6.5

58. Chemical equilibrium is referred to as dynamic because, at equilibrium, the

Reactants and products keep reacting

Equilibrium constant changes

Rates of the forward and backward reactions change

Concentrations of the reactants and products continue to change

59. Units of Kc is

Moles⁺² dm¯⁶

Kc may or may not have units

Moles² dm⁺⁶

Moles¯² dm⁺⁶

60. The product of [0H¯][H⁺] at 25C° is

10¯¹⁴

10¯²⁰

10¯¹⁰

10¹⁰

61. In a reversible chemical reaction having two reactants in equilibrium, if the concentration of the reactants are doubled then the equilibrium constant will

Becomes one fourth

Also be doubled

Be halved

Remains the same

62. A chemical reaction A ⇌ B is said to be in equilibrium when

Conversion of A to B is only 50% complete

The rate of transformation of A to B is just equal to rate of transformation of B to A in the system.

Complete conversion of A to B has taken place

Only 10% conversion of A to B has taken place

63. The factor which changes equilibrium constant o the reaction A₂(g) + B₂(g) → 2 AB(g) is

Amounts of A₂ and B₂

Catalyst

Temperature

Total pressure

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Maan AliLast Updated: April 19, 2025

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ECAT Chemistry Chemical Equilibrium Test Online

Chemistry Chemical Equilibrium MCQS Online Test

ECAT Chemistry Chemical Equilibrium Chapter Online Test

ECAT Chemistry Chemical Equilibrium Test

Chemistry

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Chemistry Chemical Equilibrium MCQS Online Test

ECAT Chemistry Chemical Equilibrium Chapter Online Test

ECAT Chemistry Chemical Equilibrium Test

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